Question

consider the following chemical equilibrium:

n₂(g) + 3h₂(g) ⇌ 2nh₃(g)

now write an equation below that shows how to calculate k_c from k_p for this reaction at an absolute temperature t. you can assume t is comfortably above room temperature. if you include any common physical constants in your equation be sure you use their standard symbols, found in the aleks calculator.

k_c =

Explanation:

Step1: Recall the relationship between \(K_p\) and \(K_c\)

The general formula is \(K_p = K_c(RT)^{\Delta n}\), where \(\Delta n\) is the change in the number of moles of gas.
For the reaction \(N_2(g)+3H_2(g)
ightleftharpoons 2NH_3(g)\), \(\Delta n=n_{products}-n_{reactants}=(2)-(1 + 3)=- 2\).

Step2: Solve for \(K_c\) from \(K_p = K_c(RT)^{\Delta n}\)

Rearrange the formula \(K_p = K_c(RT)^{\Delta n}\) to get \(K_c=\frac{K_p}{(RT)^{\Delta n}}\).
Substitute \(\Delta n=-2\) into the equation, we have \(K_c = K_p(RT)^{2}\).

Answer:

\(K_c = K_p(RT)^{2}\)